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10. Arrange the following in order of increasing boiling point and explain your reasoning (hint: structures shown are skeletal structures and may not show the complete picture) Explain your answer, being sure to use the ideas of forces and energy. A B D нн H H нн H H H-C-C-OH H-C-C-H HO-c-c-OH но-с-с-он H-C-H H-C-OH нн нн

10. Arrange the following in order of increasing boiling point and explain your reasoning (hint: structures shown are skeletal structures and may not show the complete picture) Explain your answer, being sure to use the ideas of forces and energy. A B D нн H H нн H H H-C-C-OH H-C-C-H HO-c-c-OH но-с-с-он H-C-H H-C-OH нн нн

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question 10:** **Arrange the following in order of increasing boiling point and explain your reasoning (hint: structures shown are skeletal structures and may not show the complete picture).** **Explain your answer, being sure to use the ideas of forces and energy.** Structures: - **A:** CH₃CH₂CH₂CH₃ - **B:** CH₃CH₂CH₃ - **C:** CH₃OH - **D:** CH₄ - **E:** CH₃CH₂OH ### Explanation: When arranging substances in order of increasing boiling point, consider the types of intermolecular forces present and the molecular structure. 1. **CH₄ (D):** Methane has the lowest boiling point due to its small, non-polar molecular structure, which only exhibits weak London dispersion forces. 2. **CH₃CH₂CH₃ (B):** Propane has a higher boiling point than methane because it is a larger non-polar molecule with stronger London dispersion forces than methane. 3. **CH₃CH₂CH₂CH₃ (A):** Butane, being a larger non-polar molecule than propane, will have even stronger London dispersion forces, resulting in a higher boiling point. 4. **CH₃OH (C) and CH₃CH₂OH (E):** Both methanol and ethanol exhibit hydrogen bonding due to the hydroxyl groups, which significantly increase the boiling point. Ethanol, being the larger molecule, has stronger London dispersion forces in addition to hydrogen bonding, giving it a higher boiling point than methanol. ### Order of Increasing Boiling Point: **D (CH₄) < B (CH₃CH₂CH₃) < A (CH₃CH₂CH₂CH₃) < C (CH₃OH) < E (CH₃CH₂OH)**
Transcribed Image Text:**Question 10:** **Arrange the following in order of increasing boiling point and explain your reasoning (hint: structures shown are skeletal structures and may not show the complete picture).** **Explain your answer, being sure to use the ideas of forces and energy.** Structures: - **A:** CH₃CH₂CH₂CH₃ - **B:** CH₃CH₂CH₃ - **C:** CH₃OH - **D:** CH₄ - **E:** CH₃CH₂OH ### Explanation: When arranging substances in order of increasing boiling point, consider the types of intermolecular forces present and the molecular structure. 1. **CH₄ (D):** Methane has the lowest boiling point due to its small, non-polar molecular structure, which only exhibits weak London dispersion forces. 2. **CH₃CH₂CH₃ (B):** Propane has a higher boiling point than methane because it is a larger non-polar molecule with stronger London dispersion forces than methane. 3. **CH₃CH₂CH₂CH₃ (A):** Butane, being a larger non-polar molecule than propane, will have even stronger London dispersion forces, resulting in a higher boiling point. 4. **CH₃OH (C) and CH₃CH₂OH (E):** Both methanol and ethanol exhibit hydrogen bonding due to the hydroxyl groups, which significantly increase the boiling point. Ethanol, being the larger molecule, has stronger London dispersion forces in addition to hydrogen bonding, giving it a higher boiling point than methanol. ### Order of Increasing Boiling Point: **D (CH₄) < B (CH₃CH₂CH₃) < A (CH₃CH₂CH₂CH₃) < C (CH₃OH) < E (CH₃CH₂OH)**
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